Determine the concentration of hydronium and hydroxide ions in a solution that has a pH of 1.6.

The answer to your question is [H₃O⁺] = 0.025   [OH⁻] = 3.98 x 10⁻¹³

Explanation:

Data

[H⁺] = ?

[OH⁻] = ?

pH = 1.6

Process

Use the pH formula to calculate the [H₃O⁺], then calculate the pOH and with this value, calculate the [OH⁻].

pH formula

pH = -log[H₃O⁺]

-Substitution

1.6 = -log[H₃O⁺]

-Simplification

[H₃O⁺] = antilog (-1,6)

-Result

[H₃O⁺] = 0.025

-Calculate the pOH

pOH = 14 - pH

-Substitution

pOH = 14 - 1.6

-Result

pOH = 12.4

-Calculate the [OH⁻]

12.4 = -log[OH⁻]

-Simplification

[OH⁻] = antilog(-12.4)

-Result

[OH⁻] = 3.98 x 10⁻¹³

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation: